Calculate the mole fraction of pure liquid $B$ in solution if total vapour pressure of solution,vapour pressure of pure liquid $A$ and vapour pressure of pure liquid $B$ are $500 \ mmHg$,$400 \ mmHg$ and $575 \ mmHg$ respectively at given temperature.

According to Raoult's law,the relative lowering of vapour pressure for a solution is equal to which of the following?

At $50^{\circ} C$,the vapour pressure of pure benzene is $268 \ torr$. The number of moles of non-volatile solute per mole of benzene required to prepare a solution having a vapour pressure of $167 \ torr$ at the same temperature is (molar mass of benzene $= 78 \ g \ mol^{-1}$)

At a certain temperature,when some amount of glucose is dissolved in water,it is observed that the lowering in vapour pressure is $0.6 \ mm \ Hg$ for this solution. What will be the vapour pressure of the same glucose solution if its molality is $(\frac{1}{18}) \ mol \ kg^{-1}$ (in $mm \ Hg$)?

At $25^\circ C$,the vapor pressure of $CCl_4$ is $143 \ mm \ Hg$. If $0.5 \ g$ of a non-volatile solute (molar mass $= 65 \ g/mol$) is dissolved in $100 \ mL$ of $CCl_4$,the vapor pressure of the resulting solution is $...... \ mm \ Hg$. (Density of $CCl_4 = 1.58 \ g/cm^3$)

The vapor pressure of water at $300 \, K$ is $12.3 \, kPa$. Calculate the vapor pressure of a $1 \, molal$ solution containing a non-volatile solute. (in $, kPa$)